Given that 3.33 g of the gas, at 95 °C and 790 torr, occupy a volume of 1.365 L, it is chlorine gas (Cl2).
We will start by counting the amount of moles of the gas. This can be done as follows:
(V) = 1.365 L,
(T) = 95 °C,
(P) = 790 torr,
(n) =?
(T) = 95 + 273 = 368 K
(P) = 790 / 760 = 1.039 atm
(R) = 0.0821 atm
PV = nRT
1.039 * 1.365 = n * 0.0821 * 368
n = 0.0469 mole L/Kmol
Finally, we will ascertain the gas's identity as follows:
n = 0.0469 mole
M = 3.33 g
Molecular mass =?
Molar mass is equal to the product of the mass and the mole.
Molar mass equals 3.33 minus 0.0469
Gas molar mass = 71 g/mol
As a result, we can infer that the gas is chlorine gas (Cl2) because
(Cl) = 35.5 g/mol.
(Cl2) = 2 * 35.5 g/mol
= 71 g/mol
To know more about identity of gas, visit:
https://brainly.com/question/16016861
#SPJ4
